Reaction: 1 A + 1B = 3C The initial [A] is 1.20 M and [B] is 1.50 M. The equilibrium constant is 0.0000076. What is the concentration of C at equilibrium? You may assume the 5% rule is valid.

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Chapter1: Chemical Foundations
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**Chemical Equilibrium Problem:**

**Reaction:** 
\[ 1 \, \text{A} + 1 \, \text{B} \rightleftharpoons 3 \, \text{C} \]

**Given:**
- The initial concentration of \([\text{A}]\) is 1.20 M.
- The initial concentration of \([\text{B}]\) is 1.50 M.
- The equilibrium constant (\(K_c\)) is 0.0000076.

**Problem:**
What is the concentration of \([\text{C}]\) at equilibrium?

**Note:** You may assume the 5% rule is valid for this calculation. 

In solving this problem, utilize the equilibrium expression derived from the balanced chemical equation and apply the 5% rule to simplify your calculations if applicable.
Transcribed Image Text:**Chemical Equilibrium Problem:** **Reaction:** \[ 1 \, \text{A} + 1 \, \text{B} \rightleftharpoons 3 \, \text{C} \] **Given:** - The initial concentration of \([\text{A}]\) is 1.20 M. - The initial concentration of \([\text{B}]\) is 1.50 M. - The equilibrium constant (\(K_c\)) is 0.0000076. **Problem:** What is the concentration of \([\text{C}]\) at equilibrium? **Note:** You may assume the 5% rule is valid for this calculation. In solving this problem, utilize the equilibrium expression derived from the balanced chemical equation and apply the 5% rule to simplify your calculations if applicable.
Expert Solution
Step 1

While calculating the concentrations of the individual components in an equilibrium, the amount of reactant dissociated, say ‘x’ by a time, ‘t’, then the subtracting x from the value of initial concentration is not necessary if, x is less than or equal to 5%.

 

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